Net Ionic Equations

A net ionic equation shows only the species that actually participate in a chemical reaction, omitting spectator ions that remain unchanged.

Key Concepts

• Spectator ions: Ions present in solution that do not take part in the reaction
• Molecular equation: Shows all reactants and products as compounds
• Ionic equation: Shows all strong electrolytes dissociated into ions
• Net ionic equation: Eliminates spectator ions to focus on the chemical change

Steps to Write Net Ionic Equations

1. Write the balanced molecular equation.
2. Dissociate all strong electrolytes into ions.
3. Identify and cancel spectator ions.
4. Write the resulting net ionic equation.

Example

• Molecular equation:
  NaCl(aq) + AgNO₃(aq) → AgCl(s) + NaNO₃(aq)

• Ionic equation:
  Na⁺(aq) + Cl⁻(aq) + Ag⁺(aq) + NO₃⁻(aq) → AgCl(s) + Na⁺(aq) + NO₃⁻(aq)

• Net ionic equation:
  Ag⁺(aq) + Cl⁻(aq) → AgCl(s)

Importance

• Focuses on the actual chemical change
• Simplifies analysis of precipitation, acid-base, and redox reactions
• Useful in stoichiometry calculations and predicting reaction outcomes

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